# At standard pressure, CH_4 boils at 112 K and H_2O boils at 373 K. What accounts for the higher boiling point of H_2O at standard pressure?

Between water molecules, hydrogen bonding operates, which is a potent intermolecular force. The $H - O$ bond is quite polar, i.e. ""^(delta+)H-O^(delta-)-H^(delta+), and the dipoles can align. No such intermolecular force operates between methane molecules, (because the $C - H$ bond is reasonably non-polar), and the boiling point of methane is substantially reduced with respect to water.